Sulfur hexafluoride has an octahedron structure.
No. A molecule of octahedral shape is always non-polar
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
SF6 is non-polar. Reason: Fluorine is more electronegative than sulfur, so the bond dipoles point toward fluorine. However, all the six S-F bonds are arranged octahedrally around the central sulfur. F F \ / F-S-F / \ F F Because the octahedral geometry is symmetrical, the bond dipoles cancel each other, and the molecule is nonpolar, meaning that µ = 0. Source: Another Qs from the same topic (SF6 from wikiANSWERS) which quotes the source as: "Straight from Chemistry: The Central Science. 11e. Brown/LeMay/Bursten/Murphy"
it shows tetrahedral geometry for the electron pairs geometry and trigonal pyramid the molecular geometry.
Sulfur hexafluoride has an octahedron structure.
7. Selenium hexafluoride is SeF6 , an octahedral molecule similar to SF6
The neutral SF6 molecule has no dipole moment. The gas phase SF6- ion is not that well understood- on the basis that the shape is distorted octahedral a small dipole would be expected.
No. A molecule of octahedral shape is always non-polar
sp3d2 hybridization. Example: sulfur hexafluoride (SF6)
179 and 103 degrees source and excellent explanation: http://www.madsci.org/posts/archives/2001-02/983324692.Ch.r.html
This seems like a misprint. IF6 will have one electron too many to attain an octahedral structure with 90 degree bond angles. SF6 is octahedral, for example, and does have 90 degree angles, as does PF6(-1). Perhaps IF6(+1) is the molecule in question, which will have the proper number of electrons.
SF6 is non-polar. Reason: Fluorine is more electronegative than sulfur, so the bond dipoles point toward fluorine. However, all the six S-F bonds are arranged octahedrally around the central sulfur. F F \ / F-S-F / \ F F Because the octahedral geometry is symmetrical, the bond dipoles cancel each other, and the molecule is nonpolar, meaning that µ = 0. Source: Another Qs from the same topic (SF6 from wikiANSWERS) which quotes the source as: "Straight from Chemistry: The Central Science. 11e. Brown/LeMay/Bursten/Murphy"
electron-pair geometry is octahedral with no LPs and the molecule geometry is octahedral
Sulfur hexafluoride (SF6) has a molecular shape that is octahedral. In this structure, the sulfur atom is at the center, surrounded symmetrically by six fluorine atoms located at the vertices of an octahedron. The bond angles between the fluorine atoms are approximately 90 degrees. This symmetrical arrangement contributes to the molecule's stability and non-polar characteristics.
SF6
Every pair of electrons on the central atom (S) of the Lewis structure of SF6 is shared by an F atom, so therefore there are no lone pairs on the central atom.